The distance between the nuclei of two atoms forming a covalent bond is called the bond length. Which one of the following factor affects the bond lenght?
Correct answer: D. All can affect.
- A. Electronegativity
- B. Size of the atoms
- C. Bond order
- D. All can affect.
Explanation
Option D is correct.The greater the difference in electronegativity between the two atoms, the shorter the bond length. This is because the more electronegative atom will have a greater pull on the shared electrons, which will bring the two atoms closer together. The larger the atoms, the longer the bond length. This is because the larger atoms have larger electron clouds, which means that the shared electrons are more spread out.The greater the bond order, the shorter the bond length. This is because a higher bond order means that there are more shared electrons, which brings the two atoms closer together.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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